Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: interminable on March 26, 2010, 02:50:56 PM
-
In lab we synthesized copper (II) acetate starting from copper (II) sulfate pentahydrate. First ammonia was added, followed by sodium hydroxide.
I've been working on the balanced equations, and I understand we're forming a Cu(OH)2 precipitate twice, (we dissolved it with excess ammonia the first time and reformed it with the NaOH).
We dissolve the Cu(OH)2 in 10% acetic acid solution to obtain the acetate product. I'm just wondering why dissolving the copper (II) sulfate directly in the acetic acid and skipping all the other steps wouldn't work.
-
If you were to add acetic acid directly, then the reaction (supposing that they react) would be :
CuSO4 + CH3COOH :rarrow: (CH3COO)2Cu + H2SO4
But as you can see, a weak acid (acetic acid) is displacing a stronger acid (sulphuric acid) from its salt. That's not possible.
On the other hand, when you add NaOH, the acid being displaced is H2O, which is certainly weaker than acetic acid. (wirte the equation)
P.S : I recently learned on this forum that there might be rare exceptions to this rule. http://www.chemicalforums.com/index.php?topic=40518.0
-
Thanks, the answer seems obvious now, haha.
Cu(OH)2 + CH3COOH --> Cu(CH3COO)2 + H2O
This is what you were referring to, right?
-
Yes